Removal and recovery of sulfur oxides from gases

ABSTRACT

A PROCESS FOR REMOVING SULFUR OXIDES FROM GAS STREAMS WHEREBY THE SULFUR OXIDES ARE ADSORBED ONTO A CARBONACEOUS ADSORBENT AND RECOVERING SULFUR DIOXIDE FROM THE SPENT ADSORBENT BY CONTACTING THE ADSORBENT WITH AN OXIDE-REDUCING GAS, I.E., HYDROGEN SULFIDE, WHEREBY THE ADSORBED SULFUR OXIDES HAVING BEEN ADSORBED AS SULFURIC ACID AND SULFUR TIOXIDE ARE REDUCED TO SULFUR DIOXIDE AND ELEMENTAL SULFUR, THEN REMOVING THE ELE-   MENTAL SULFUR FROM THE ADSORBENT BY CONTACTING WITH A SULFUR-REDUCING GAS AND THEREAFTER RECYLCING THE ADSORBENT.

Feb. 16, 1971 s. L. ToRRENcE 3,563,704

REMOVAL AND RECOVERY OF SULFUR OXIDES FROM GASES Filed Aug. l5, 1968 2 Sheets-Sheet 2 f/l/ I 50a 700506552 t/ ,z3/ery n Uf 6,05 jg #OJ r me@ ou V f/Z S04.

QECOVEZED SOZ /22j 1 V75 rl United states Patent o 3,563,704 REMOVAL AND RECOVERY OF SULFUR OXIDES FROM GASES Samuel L. Torrence, Charleston, S.C., assignor to Westvaco Corporation, New York, N.Y., a corporation of Delaware Filed Aug. 13, 1968, Ser. No. 752,298 Int. Cl. C011) 17/60, 17/16 U.S. Cl. 23-178 11 Claims ABSTRACT OF THE DISCLOSURE This invention relates to a process for removing sulfur oxides from oxygen-containing gas streams by adsorption onto a carbonaceous adsorbent and recovering sulfur dioxide from the spent adsorbent. More specifically, this invention relates to removal of sulfur dioxide and sulfur trioxide from flue gases by adsorbing the oxides onto an activated carbon and regenerating the spent carbon by contacting first with hydrogen sulfide and subsequently contacting iwith a sulfur-reducing gas. The regenerated adsorbent is then recycled to the sulfur oxide adsorber and sulfur dioxide is recovered.

Many industrial plants employed fuels having a sulfurcontent as high as three percent or more. These fuels, primarily coal and fuel oil, upon combustion, form undesirable pollutants, including sulfur oxides. Removal of these sulfur oxidesfrom eiiluent gas streams has long been a troublesome problem. The economic advantages of this invention enable power plants to use high sulfurcontent fuels without fear of air pollution. In addition, other industrial efliuents, such as those from pulp mills, contribute to sulfur oxide pollution. For the purposes of this invention, sulfur oxides are herein defined as sulfur trioxide and sulfur dioxide. The presence of these sulfur oxides in waste gases passed into the atmosphere results in considerable amounts of pollution.

The removal of sulfur oxides from flue gases may be achieved by chemical or physical processes, using liquid or solid substances. The most successful combinations of these processes are wet scrubbing with liquids and dry methods which employ contacting with solid substances. The objective of all the processes is to prevent the emission of the noxious and offensive sulfur oxide gases into the atmosphere. Wet scrubbing lowers the temperature of the gas stream to that of the washing water, which is considerably lower than the temperature necessary to retain the buoyancy necessary to disperse the emissio-n over a wide area. In contrast, dry processes have the advantage over wet processes of maintaining a high emission temperature.

The dry processes contact adsorbent material with the gases to be cleaned. In order to keep the adsorbent inventory at a minimum and the plant from being excessively large, the adsorbent must have a high adsorbing efficiency. High efficiency means a high gas throughput per unit volume of adsorbent in the contacting equipment. In addition, the adsorbent must be relatively hard with minimum attrition; most importantly, the adsorbent ice must be easily and inexpensively regenerated. Included among the several dry processes that have been developed are a catalytic oxidation process (U.S. Pat. 3,318,662), a manganese nodule process (U.S. Pat. 3,330,096), an alkalized alumina process, (U.S. Pat. 2,992,884) and activated char processes (U.S. Pat. 2,992,895 and 2,992,065 One of the major costs in these dry processes is the charge for material used to react with the sulfur oxides. For instance, in the alkalized alumina process producer gas is the reactant; whereas in the activated char process the reactant is the carbonaceous adsorbent itself. One of the principal disadvantages of these processes, particularly the activated char process, is the expensive regenerating costs. A difficulty in developing an economical process is that large volumes of gas conltaining low concentrations of sulfur oxides, i.e., on the order of 0,1 to 5.0 percent by volume must lbe processed. Because of this difficulty the activated char process has the disadvantage of being forced to use large adsorber sizes.

The activated char process removes sulfur oxides from a gas stream by using a carbonaceous adsorbent, such as an activated char, long recognized as a good adsorbent. In this process the activated char catalytically oxidizes sulfur dioxide to sulfur trioxide which is adsorbed as such, or is combined with water vapor to form sulfuric acid, both of which adhere tightly to the surface of the activated char. In the normal combustion of fuels there are present in the ue gas amounts of oxygen and water in excess of that needed to carry out the oxidation of sulfur dioxide and the hydration of the resulting sulfur trioxide to form sulfuric acid. The spent char is then regenerated at temperatures above 300 C., whereupon the sulfuric acid splits into water and sulfur trioxide, the lato ter being reduced to sulfur dioxide with the carbonaceous adsorbent serving as a reducing agent. One of the disadvantages of this process is that the carbonaceous adsorbent is used as the reducing agent, therefore large losses of adsorbent, known as burn-olf, occur. Regeneration is carried out according to the following reaction:

Consumption of an activated carbon at the rate needed for regeneration according to Reaction l, i.e., about 0.1 pound of carbon per pound of sulfur dioxide recovered, is economically unattractive. Because of the necessity of replacing a substantial portion of the adsorbent with each adsorption and regeneration cycle, it is necessary that an inexpensive char be employed. These chars generally have low adsorption rate and capacity characteristics necessitating large adsorber sizes to compensate for these poor characteristics. Another disadvantage is that the inexpensive char, which has a low hardness, becomes structurally weaker and more subject to attrition as a. result of burn-off during regeneration.

The usual regeneration treatment is to heat the spent adsorbent which causes the sulfur trioxide to react with `the adsorbent in accordance with Reaction 1, thereby producing a concentrated stream of sulfur dioxide; whereas, another process washes the adsorbent with water to remove the adsorbate as dilute sulfuric acid. Therefore, chemical reduction is the preferred regeneration method because a concentrated stream of sulfur dioxide is recovered as a 40% to 50% gas mixture which can be processed economically in that state or used as a raw material for the production of sulfur or sulfuric acid.

It is a general object of this invention to provide a process for regenerating a carbonaceous adsorbent having sulfur oxides adsorbed thereon without consuming the adsorbent, A more specific object is to provide a continuous process for removing sulfur dioxide and sulfur trioxide from flue gases whereby the oxides are adsorbed onto activated carbon and the spent carbon is then contacted with an oxide-reducing gas which will `reduce the adsorbate to sulfur dioxide and sulfur, without burn-off losses. For the purpose of this invention the term adsorbate is construed to mean adsorbed sulfur trioxide, adsorbed sulfuric acid, and varying amounts of both sulfuric acid and sulfur trioxide. Another object is to provide a process for regenerating spent carbon by sequentially contact the carbon with an oxide-reducing gas to recover sulfur dioxide and then with a sulfur-reducing gas to remove sulfur from the adsorbent. A further object is to provide a regenerating process employing a hard granular activated carbon possessing high rate and capacity characteristics. A still further object is to provide a process for sequential removal of sulfur trioxide and sulfur dioxide, thereby permitting the gas stream to pass to the atmosphere free from sulfur oxide pollution.

For the purposes of the instant invention, the term oxide-reducing gas is defined to mean all compounds which will reduce adsorbed sulfur trioxide (S03) per se or in the hydrated form as sulfuric acid, to sulfur dioxide (SO2). Stich compounds include hydrogen sulfide (H28) and carbonyl sulfide (COS). By the term sulfur-reducing gas it is intended to denote those compounds which will reduce elemental sulfur and include hydrogen (H2) and carbon monoxide (CO). Thus, it may be seen that any number of sulfur-reducing gases may be used which include hydrogen, producer gas and reformed natural gas.

It has now been found that removal of adsorbed sulfur oxides from spent carbonaceous adsorbent may be accomplished without carbon burn-off by contacting the adsorbent with an oxide-reducing gas, preferably hydrogen sulfide. Spent adsorbent is the term used to described the condition of the adsorbent after it has adsorbed sulfur oxides from a gas stream as sulfur trioxide and sulfuric acid, or a combination of both. Spent adsorbent is contacted with an oxide-reducing gas whereby the adsorbate is reduced to sulfur dioxide and sulfur, and sulfur dioxide is continuously purged from the regenerator. In a preferred method, the adsorbent having sulfur deposited thereon is contacted with sulfur-reducing gas to remove the adsorbed sulfur and the thus regenerated adsorbent is then recycled to the sulfur oxide adsorber. It has also been found that the use of this preferred method allows utilization of a hard granular carbon having superior adsorption rate and capacity characteristics and a low attrition rate as the adsorbent. The adsorption and regeneration may be carried out in a fixed bed system or a continuously moving bed system, but the preferred process utilizes a uidized bed system wherein the carbon adsorbent is continuously circulated through the system.

The dirty flue gas is passed countercurrent to the continuously moving carbon adsorbent and the sulfur oxides are adsorbed therefrom. The sulfur oxide removal efficiency of the process can be designed to be as high as required, for example, the gas stream as it passes to the atmosphere may be reduced to less than 5 p.p.m. of sulfur from an initial concentration of 1,000 to 50,000 p.p.m. However, for economic reasons, it is usually preferable to adsorb about 90% of the sulfur oxides from the gas stream.

The liuc gas entering the sulfur oxide adsorber may contain sizeable amounts of solid materials such as y ash and dust. This material does not noticeably impair the adsorption characteristics of the activated carbon when a uidized bed system is used because the adsorption bed is in a dynamic state.

Physical adsorption of sulfur dioxide by activated carbon at flue gas temperatures is very low, but sulfur trioxide by comparison is readily adsorbed. Consequently, satisfactory removal from the gas stream depends upon the carbon acting as a catalyst in the oxidation of sulfur 4 dioxide to sulfur trioxide which is hydrolyzed to sulfuric acid if water vapor is present in the flue gas. The oxygen and water vapor necessary for the reaction are normally present in the ue gas, but they may be added if desired. The sulfuric acid thus formed is retained on the carbon surface and in this manner sulfuri oxides are removed.

carbon One of the advantages of an activated carbon process is that sulfur oxide removal may be performed at flue gas temperatures. The lower sulfur oxide adsorption temperature is kept above 200 F. in order to retain buoyancy. The upper adsorption limit is determined by the reaction and ignition characteristics of the particular carbon used. For one particular carbon the adsorption of sulfur oxides takes place at temperatures up to about 350 F. Where corrosion problems are not a factor the adsorption of both sulfur trioxide and sulfur dioxide, as sulfur trioxide or sulfuric acid, may be accomplished simultaneously. The preferred temperature for sulfur oxide adsorption is between 200 F. and 260 F. in order to retain buoyancy and satisfactory adsorption rate and capacity characteristics. If buoyancy is not a factor the adsorption make take place at temperatures below 200 F. In adsorber units where corrosion by sulfur trioxide is a problem the adsorption of sulfur oxides is performed sequentially, using a single adsorbent so as to first adsorb the sulfur trioxide while it is at a temperature above its dew point and then to oxidize and adsorb the sulfur dioxide as mentioned above. The dew point of sulfur trioxide in most fiue gases ranges between 250 F. and 480 F., which is much higher than the dew point of sulfur dioxide. Because of this difference, it is desirable to adsorb sulfur trioxide in one portion of the adsorber at a temperature above the dew point of sulfur trixoide, preferably between 300 F. and 350 F., and adsorb sulfur dioxide in another portion of the adsorber at a temperature below the dew point of sulfur trioxide, preferably 200 F. to 260 F.

Any carbonaceous adsorbent may be used in the process of this invention, but an activated carbon is preferred. Since the regeneration procedure does not consume the activated carbon adsorbent, a highly activated, more effective hard carbon, such as those disclosed in co-pending application S.N. 734,566, may be used. Through the ability to use the more highly activated carbons, the throughput of gas per volume of carbon can be increased by ve to seven times more than the throughput with activated char. This achievement means a significant reduction in the size of the adsorption equipment required for a sulfur dioxide recovery process. In addition, hard activated carbons are much less subject to abrasion than are chars, the result being lower attrition losses.

The essence of this invention is that regeneration may be efficiently carried out by using hydrogen sulfide as the oxide-reducing gas for recovering sulfur dioxide from spent carbons. Although a number of reactions may be postulated under the proper regeneration conditions the stoichiometry is described by the following reactions:

carbon (3] II- YS O1 -tllgS S Og S -t- BH3() carbon [4] ILSO., BIDS 4S -t- 41h() The carbon burn-off during these regenerations is negligiblc and the sulfur formed by Reactions 3 and 4 remains absorbed on the carbon surface. It is believed that the carbon acts as a catalyst not only in the adsorption of sulfur oxides but in the regeneration as well. The proportions of Reactions 3 and 4 occurring is a function of the regenerating temperature, which may be varied between ambient temperature and 570 F. It has been found that when using one particular carbon at temperatures below 250 F. Reaction 4 predominates and sulfur remains adsorbed on the carbon. As the regeneration temperature is raised above 250 F. Reaction 3 is favored and the percentage of sulfur doixde evolved is increased. It has been shown that although regeneration may be carried out at temperatures above 570 F., complete sulfur trioxide and sulfuric acid reduction may be acomplished at temperatures below 570 F. The sulfur dioxide formed is continuously purged and conveyed from the regenerator to further processing for sale as indicated above. When using carbonyl sulde as the oxide-reducing gas, an analogous set of reactions for the reduction of the adsorbate may be made.

The treated adsorbent having sulfur on its surface is carried to a second regenerator to remove the adsorbed sulfur. The adsorbed sulfur may be removed by a variety of sulfur-reducing gases, but the preferred sulfur-reducer is hydrogen.

carbon a The hydrogen sulfide formed by this reaction is carried to the first regenerator for use in Reactions 3 and 4. The regenerated carbon is then recycled without any loss in effectiveness for adsorption of sulfur oxides. It is desirable to carry ont Reaction 5 at temperatures above 500 F. It has been found that temperatures between 800 F. and 1300 F. satisfactorily remove the elemental sulfur at a sufiiciently short reaction time, but lower temperatures may be used if sufficient reaction time is allowed. The complete regeneration is preferably conducted by chemical reduction of the adsorbate to sulfur dioxide and elemental sulfur by hydrogen sulfide, and reaction of adsorbed elemental sulfur with hydrogen to form hydrogen sulde. Thus the hydrogen sulfide which is required for reduction of sulfuric acid in Reactions 3 and 4 is formed within the system by the reaction of adsorbed elemental sulfur with hydrogen. Examination of the chemistry shown below reveals that the overall regeneration can be summarized as a hydrogen reacting with sulfuric acid to produce sulfur dioxide and hydrogen sulfide (Reactions 6 and 7).

HgS -i- 4 H2O A second method for removing elemental sulfur from the adsorbent is to use carbon monoxide as the sulfurreducing gas as in Reaction 9 to form COS, and catalytically convert the COS to HZS as in Reaction 10 before contacting the oxide-reducing gas with the adsorbate.

albon c. [n] oo s cos catalyst [10] Cos H20 His CO2 A third method for removing elemental sulfur from the carbon adsorbent is to convert carbon monoxide to hydrogen by the commonly practiced water-gas shift reaction shown by Reaction 11.

6 The hydrogen thus produced is contacted with the sulfurcontaining carbonaceous adsorbent and Reaction 5 occurs.

The advantages offered by this invention include the ability to use a process whereby burn-off of activated carbon may be virtually eliminated. A second advantage is the ability to use a carbon possessing superior adsorption rate and capacity characteristics. Regeneration by chemical reduction has the further advantage of producing a stream concentrated in sulfur dioxide which can be further processed to such products as liquid sulfur dioxide, sulfuric acid or sulfur. Another advantage is that this invention may be carried out in either a fixed bed or in a continuous manner, such as in a fiuidized bed.

The above and other objects of the present invention will become more readily apparent form the folowing description of the drawings, the gures ybeing schematic flow diagrams of processes for carrying out the present invention.

FIG. 1 is a schematic drawing of the process of this invention in its broadest scope.

FIG. 2 is a schematic drawing of the process of this invention in a preferred form.

FIG. 1 of the drawings, described the process as a moving bed process for removing sulfur dioxide and hydrogen sulfide, uses these specific terms by way of reference for simplicity in showing one aspect of the invention. In FIG. 1, activated carbonaceous adsorbent 13 is fed to the sulfur dioxide adsorbert 11 and catalyzes the oxidation of sulfur oxides contained in the dirty flue gas stream 10. The adsorbent remains on the carbon surface as the gas stream passes through the adsorber countercurrent to the moving bed of adsorbent. Clean flue gas 12, having substantially all the sulfur oxides removed, or only an insignificant amount remaining, passes to the atmosphere. The carbon containing the adsorbent is moved via 15 into the regenerator 16 where it is contacted with an oxide-reducing gas, shown here as hydrogen sulfide 20. Sulfur dioxide and elemental sulfur are formed from the chemical reduction of the adsorbate according to Reaction 3, and sulfur dioxide is recovered in concentrated stream 22 suitable for further processing, or elemental sulfur only may be formed according to Reaction 4 or the conditions may be adjusted to give intermediate proportions of both sulfur dioxide and elemental sulfur. The carbonaceous adsorbent containing adsorbed elemental sulfur is removed form the regenerator at 17 and may be further processed or discarded.

FIG. 2 shows a preferred process for carrying out this invention. Activated carbon 113 is fed to the sulfur dioxide adsorber 111, wherein sulfur oxides present in the dirty flue gas are adsorbed on the carbon surface as the clean gas stream 112 passes to the atmosphere. The spent carbon 115 is removed to the H28 regenerator 116 where it is contacted with hydrogen sulfide 120. A stream of concentrated sulfur dioxide 122, formed by the chemical reduction is recovered for further processing or sale. The carbon from regenerator 116, containing adsorbed elemental sulfur, moves via 117 into reducing regenerator 118 where the adsorbent is heated and contacted with a sulfur-reducing gas 119. The preferred sulfur-reducing gas, hydrogen, reacts according to Reaction 5 to form hydrogen sulfide and the thus-formed hydrogen sulfide is carried via line 120 to supply the regeneration gas for chemical reduction of the adsorbate in regenerator 116. Excess hydrogen sulfide from regenerator 118 is removed at 121 and may be further processed to sulfur dioxide, sulfuric acid or elemental sulfur. The thus-regenerated carbonaceous adsorbent is then recycled at 113 to the sulfur dioxide adsorber and the cycle is repeated'Attrition make-up is added at 114.

The processes outlined above substantially eliminates the carbon burn-off encountered when using the acti- Vated char process, thereby allowing the use of a highly adsorbent carbon. In addition, the activated carbon upon recycle retains a constant level of effectiveness for removing sulfur oxides from gas streams.

The practice of this invention may clearly be seen in the following examples.

EXAMPLE 1 The amount of burn-off of activated carbon during regeneration was determined by first treating a spent adsorbent with hydrogen sulfide and measuring the amount of CO and CO2 formed by the reaction of the carbon adsorbent found in the efliuent gas stream, then treating the adsorbent, which contained elemental sulfur, with hydrogen and measuring the amount of CO and CO2 in the etiiuent stream formed during the reduction of the sulfur.

A degree of adsorption of 12 grams of sulfur dioxide per 100 grams of carbon was chosen. The sulfur dioxide was adsorbed from a simulated fine gas stream having the following composition: l,

Component: Percent by volume so2 0.3 O2 3.4 H20 6.9 CO2 11.6 `N2 Adsorption was carried out in a one-inch diameter cylindrical adsorber charged with 100 cc. of a hard granular carbon in a fixed bed. The gas stream was passed downward through the carbon bed at a temperature of 203 F. and a space velocity of 200G/hr. until 12 grams of sulfur dioxide was adsorbed as sulfuric acid.

Regeneration was carried out by exposing the spent carbon to a stream of H28, at a concentration of 11.6% by volume in a helium carrier. The helium was used as a carrier to simplify analytical procedures, but in practice any inert gas would be suitable. The regeneration was begun at ambient temperature with the temperature increasing steadily to 450 F. in 150 minutes. The space velocity was 1Z0/hr., which is equivalent to a gas-contact time of approximately seconds at 450 F. The efiiuent gas stream was monitored so SO2, HES, CO and CO2. The amounts of gases were measured quantitatively and the amounts of CO and CO2 in the efiiuent gas stream were used to determine the amount of carbon burn-off. Analysis for CO and CO2 showed that carbon burn-off was l mole carbon per 100 moles of adsorbed sulfur dioxide, whieh is a burn-off of 0.02% of the carbon adsorbent. Analysis of the efiiuent stream for recovered SO2 showed that 86% of the adsorbed sulfuric acid was recovered with the rest remaining adsorbed as elemental sulfur.

The adsorbent having elemental sulfur adsorbed thereon was then contacted with hydrogen gas starting at ambient temperature and increasing to 1150 F. in 180 minutes. The space velocity was 145 /hr. or a gas-contact time of approximately 3 seconds of 1150 F. An analysis of' the effluent gas stream showed the hydrogen reacted to form hydrogen sulfide, thus removing sulfur from the carbon. The carbon burn-off was 2.5 moles carbon per 100 moles of adsorbed sulfur dioxide.

EXAMPLE 2 The effectiveness of carbon upon regeneration was tested by measuring the efficiency in removing SO2 from the adsorber gas stream. Thus, any changes in the carbons ability to adsorb SO2` would be reflected by a decrease in the measured efficiency.

A recycle series using hydrogen sulfide followed by hydrogen for regeneration was continued through seven cycles following the procedure of Example 1. The data shown in the table below indicate that the carbon remains 95-l00% efficient in recovering approximately 12 g. sulfur dioxide per 100 g. carbon at 203 F. and a space velocity of 200G/hr.

RECYCLE OF CARBON REGENERATED TH HQS AND H2 according to Reaction 3 increased from 66% in Cycle 4 to 84% in Cycle 5 because the regeneration temperature rate was increased. In Cycle 4, the temperature was raised to 350 F. in 8O minutes, Whereas in Cycle 5, 350 F. was reached in 2O minutes. In Cycles 6 and 7, 350 F. was reached in 15 and 17 minutes respectively, but there was little change in sulfur dioxide recovered. These data indicate that higher regeneration temperatures favor Reaction 3 and consequently encourage sulfur dioxide formation and lower consumption of hydrogen sulfide and hydrogen. The highest burn-off occurred in Cycle 6 which was also the cycle with the fastest temperature increase.

In the hydrogen regeneration of Cycle 7, the maximum temperature was lowered to 1150 F. from 1300 F. on previous cycles. These data indicate that the high efiiciencies in Cycles 1-7 were maintained at regeneration temperatures approaching 1300" F.

Carbon burn-off was low in each cycle of the regeneration and ranged from approximately one to four moles of carbon per 100 moles of sulfuric acid or about 2-8% of that encountered using a char process, with thermal regeneration. Put in other terms, the carbon loss at 1-4 moles of carbon per 100 moles of adsorbed sulfurie acid is about 0002-0008 pound of activated carbon used per pound of sulfur dioxide recovered.

While the invention has been described and illustrated herein by references to various specific materials, procedures, and examples, it is understood that the invention is not restricted to the particular materials, combinations of materials, and procedures selected for that purpose. Numerous variations of such details can be employed, as will be appreciated by those skilled in the art.

I claim:

1. A process for regenerating a carbonaceous adsorbent having sulfuric acid adsorbed thereon comprising:

(a) contacting the carbonaceous adsorbent having sulfurie acid adsorbed thereon with an oxide-reducing gas from the group consisting essentially of hydrogen sulfide and carbonyl sulfide at a temperature below 570 F. and sufiicient to reduce the adsorbed sulfurie acid to elemental sulfur and sulfur dioxide.,

(b) recovering said sulfur dioxide from said adsorbent containing elemental sulfur, and

(c) heating said adsorbent containing elemental sulfur with a sulfur-reducing gas from the group consisting essentially of hydrogen, carbon monoxide and hydrogen-forming gases at a temperature between 800 F. and l300 F. to reduce said adsorbed sulfur to hydrogen sulfide.

2. The process of claim 1 wherein said oxide-reducing gas is hydrogen sulde.

3. The process of claim 1 wherein said sulfur-reducing gas is hydrogen.

4. The process of claim 1 wherein said sulfur-reducing gas is carbon monoxide.

5. The process of claim 1 wherein said carbonaceous adsorbent is contacted with an oxide-reducing gas at a temperature between 250 F. and 570 F.

6. The process of claim 1 wherein said carbonaceous adsorbent is an activated carbon.

7. The process of claim 1 wherein said carbonaceous adsorbent is a continuously moving mass.

8. A continuous process for removing sulfur oxides from an oxygen-containing gas stream comprising:

(a) passing the gas stream into contact with a carbonaceous adsorbent at a temperature between 200 F. and 450 F. to adsorb the sulfur oxides onto said carbonaceous adsorbent as sulfuric acid;

(b) continuously regenerating said carbonaceous adsorbent having sulfuric acid adsorbed thereon by contacting said adsorbent with an oxide-reducing gas from the group consisting essentially of hydrogen sulfide and carbonyl sulde at a temperature between 250 F. and 570 F. for a period sucient to reduce said adsonbed sulfuric acid to sulfur dioxide and elemental sulfur;

(c) removing and recovering said sulfur dioxide from said carbonaceous adsorbent containing sulfur; and

(d) heating said adsorbent containing elemental sulfur with a sulfur-reducing gas from the group consisting essentially of hydrogen, carbon monoxide and hydrogen-forming gases at a temperature between 800 F. and 1300 F. to reduce said adsorbed elemental sulfur to hydrogen sulfide.

9. The process of claim 8 wherein said continuous process is carried out in a uidized bed.

10 10. The process as defined in claim 8, further compris- 111g;

(e) using the hydrogen sulde formed in step (d) as the oxide-reducing gas in step (b). 11. The process as dened in claim 8, further comprising;

(f) recycling the carbonaceous adsorbent from which said elemental sulfur has been reduced into contact with said gas stream.

10 References Cited UNITED STATES PATENTS 3,284,158 11/1966 Johswich 23-178 15 3,345,125 10/1967 Kruel et al. 23-178X 3,454,354 7/1969 Kerr 23-2.1

FOREIGN PATENTS 749,940 1/1967 Canada 252-411 OSCAR R. VERTIZ, Primary Examiner C. B. RODMAN, Assistant Examiner U.S. Cl. X.R. 25 23-2.1, 181, 226

gyg UNITED STATES PATENT OFFICE CERTIFICATE 0F CORRECTION Patent No. 3,563 704 Dated FebYUYy 15 a .|971

Inventods) S. L. Torrence It is certified that error appears in the above-identified patent and that said Letters Patent are hereby corrected as shown below:

Col umn l line 36 "employed" shoul d read employ Column line l3, "Contact" shoul d read contacting Column line 6 "sulfuri should read sul fur Column line 23 "make" should read may line 65 "absorbed" should read adsorbed line 75 "doixide" should read dioxide line l5, "form" should read from Column Column 4 4 Column 6 Col umn line l5 "folowing" should read fol lowing Col umn 6 line 23, "described" shoul d read describing Col umn 6 line 28, "adsorbert" should read adsorber Col umn 6 line 30 "adsorbent" should ready adsorbate Col umn 6 line 35 "adsorbent should read adsorbate Col umn 6 line 46 "form should read from Signed and sealed this 22nd day of June 1 971 (SEAL) Attest:

EDWARD M.FI..ETCHER,JR. WILLIAM E. SCHUYLER, JR. Attestng Officer Commissioner of Patents 

